What is the minimum mass of ice at 0.0 c that must be added to 1.00 kg of water to cool the water from 28.0 c to 12.0 c? (heat of fusion = 333 j/g; specific heat capacities: ice = 2.06 j/gk, liquid water = 4.184 j/gk)

175g of ice

Explanation:

The heat (Q) required to cool an amount of water is:

Q = C×ΔT×m

Where C is specific heat capacity of water (4,184J/g°C), ΔT is the change in temperature (28,0°C-12,0°C = 16,0°C) and m is mass of water, 1000g of water.

Replacing:

Q = 4,184J/g°C × 16,0°C × 1000g = 66944 J of energy.

This energy is obtained from ice that requires an energy for the fusion process and an additional energy increasing its temperature from 0.0°C to 12,0°C. That could be written as:

66944 J = 333 J/g×m + 4,184J/g°C×12,0°C×m

Where m is mass of ice.

66944 = 333m + 50.2m

66944 = 383.2m

m = 175g of ice

I hope it helps!

fire could start, buildings collapsing, and ash falling from the sky.

explanation:

this is because the buildings or plants could catch on fire and the buildings would most likely collapse. lastly ash would fall because all the burning would cause ash to fall from the sky.

hope this .

in 1783 cavendish was working with his hydrogen gas and found that when he burned it and condensed the vapor it was water. this was very significant since it disproved the greek theory of elements completely since water was not a simple substance but the product of two gases. it was lavoisier who hearing of the experiment gave cavendish's gas the name hydrogen ("water-producer") and added that hydrogen burned by combining with oxygen and that water was a hydrogen-oxygen combination.

explanation: